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Answer :
Final answer:
To calculate the equilibrium constant for the dissolution of NiCO_3, use the equation K = exp(-ΔG°/RT) with the ΔG° given in the question, R as the ideal gas constant, and T as the temperature in Kelvin. Convert ΔG° into appropriate units before calculation.
Explanation:
The question is asking about the calculation of the equilibrium constant of the dissolution of NiCO_3, given its standard free energy change. For dissolution reactions, the equilibrium constant can be calculated by using the equation: K = exp(-ΔG°/RT). In this case, ΔG° is the standard free energy change (39.1KJ), R is the ideal gas constant (8.314 J/mol K), and T is the temperature in Kelvin (298 K).
Before any calculation, it’s important to convert ΔG° into J, since the units of R are in J. So ΔG° = 39.1KJ = 39100J. Now, you can plug everything into the equation: K = exp(-39100J/((8.314 J/mol K) x 298 K)). Solving this gives you the value of the equilibrium constant.
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